2. Electron Orbitals
Heisenberg
1. The ____________ ______________ principle states that it is impossible to determine simultaneously both the position and the velocity of an electron or any other particle.
Uncertainty

3. Electron Orbitals
pauli
exclusion
1. The ______ ___________ principle states that no two electrons can have the same set of four quantum numbers.

4. Electron Orbitals
principal
a. The __________ quantum number (n), indicates the main energy level. Values of n are positive integers 1, 2, 3, and so on.

5. Electron Orbitals
angular
b. The ___________ _____________ quantum number (l) indicates the shape of the orbital.
momentum

6. Electron Orbitals
(l)
Orbital Type s 1 p 2 d 3 f

7. Electron Orbitals
magnetic
c. The ____________ quantum number (ml) indicates the orientation of an orbital around the nucleus. Can have a value of –l through zero to +l.

8. Electron Orbitals
spin
d. The _____ quantum number (ms) has only two possible values, + ½ and – ½ , because only two electrons can exist in the same orbital and indicates one of the two fundamental spin states.

9. Electron Orbitals
aufbau
2. The ________ principle states that an electron will occupy the lowest-energy orbital that can receive it.

10. Electron Orbitals
3. ________ rule states that orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbits have the same spin.
Hund’s

11. Electron Orbitals
1. The arrangement of electrons in an atom is known as the atom’s ___________ _________________. One type of electron configuration is _________ ___________.
Electron
configuration
orbital
notation